 ## Q. 3.22

The industrial process for making the ammonia used in fertilizer, explosives, and many other products is based on the reaction between nitrogen and hydrogen at high temperature and pressure:

$N_{2}(g) + 3 H_{2}(g) → 2 NH_{3}(g)$

If 18.20 kg of $NH_{3}$ is produced by a reaction mixture that initially contains 6.00 kg of $H_{2}$ and an excess of $N_{2}$, what is the percent yield of the reaction?

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